Question

How many Faradays are required for the oxidation of one mole of \( \text{H}_2\text{O} \) to \( \text{O}_2 \)?

Hint:

The number of Faradays required for a reaction is determined by the number of electrons transferred during the reaction. One mole of electrons corresponds to one Faraday.

Answer 1

The oxidation of \( \text{H}_2\text{O} \) to \( \text{O}_2 \) involves the following reaction: \[ 2 \text{H}_2\text{O} \rightarrow \text{O}_2 + 4 \text{H}^+ + 4e^- \] Since 4 electrons are involved in the oxidation of 2 moles of water, the number of Faradays required for 1 mole of \( \text{H}_2\text{O} \) to produce 1 mole of \( \text{O}_2 \) is 4. Thus, 4 Faradays are required.